A student adds 0.1 mol of phosphoric acid and 0.1 mol of sodium hydrogen oxalate

Question

A student adds 0.1 mol of phosphoric acid and 0.1 mol of sodium hydrogen oxalate (NaHC_2O_4) to enough water to make 1.0 L of solution. The following equilibrium is established with the concentrations of the reactants greater than the concentrations of the products. Which of the statements about the equilibrium system is correct? HC_2O_4^- (aq) + H_3PO_4(aq) H_2C_2O_4(aq) + H_2PO_4^- (aq) Oxalic acid is a weaker acid than phosphoric acid. The dihydrogen phosphate anion, H_2PO_4^-, is a stronger acid than oxalic acid. Phosphoric acid is a stronger acid than oxalic acid. The hydrogen oxalate anion, HC_2O_4^-, is a weaker base than the dihydrogen phosphate anion, H_2PO_4^-. Water is a stronger acid than either oxalic or phosphoric acids.

Explanation / Answer

Correct Answer- The Hydrogen oxalate anion is weaker base than the dihydrogen phosphate anion as the reactant concentration is more the reaction happens mainly in backward direction. That tells Oxalic Acid is much stronger acid than dihydrogen phosphate. And so the conjugate base will be weaker.

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.